The enthalpy change when 1 g of water is frozen at `0^@C` (`Delta_(fus) H^@=-1.435` kcal/mol) is __________ .

What is the enthalpy change when 1.0 g of water is frozen at 0^(@)C ? Delta_(fus) = H = 6.02 kJ "mol"^(-1) .

The enthalpy change when 1.00 g of water freezes at 0^(@)C and 1.00 atm is (DeltaH_("fusion")=1.435 k.cal//mol)

Calculate the enthalpy change of freezing of 1.0 mol of water at 10^(@)C to ice at -10^(@)C, Delta_(fus)H=6.03 kJ mol^(-1) at 0^(@)C . C_(P)[H_(2)O(l)]=75.3 J mol^(-1) K^(-1) C_(P)[H_(2)O(s)]=36.8 J mol^(-1) K^(-1)

The enthalpy change of freezing of 1 mol of water at 5^(@)C to ice at -5^(@)C is (Given Delta_(fus)H=6kJ"mol"^(-1) at 0^(@)C , (C_(p)(H_(2)O,s)=36.8J"mol"^(-1)K^(-1))

The enthalpy change on freezing of 1.0 mol of water at 10^(@)C to ice at -10^(@)C is : Delta_(fus). H^(@)=6.03 kJ mol^(-1) at 0^(@)C C_(p)[H_(2)O(l)]=75.3 J mol^(-1)K^(-1) C_(p)[H_(2)O(s)]=36.8 J mol^(-1) K^(-1)

Calculate enthalpy change on freezing 1 mol water at 10^(@)C to ice at -10^(@)C. Delta_("fus")H= 6.03 " kJ mol"^(-1) " at " 0^(@)C . C_(p)[H_(2)O(l)]= 75.3 " J. mol"^(-1). K^(-1) , C_(p)[H_(2)O(s)]= 36.8 " J mol"^(-1). K^(-1) .

Calculate the enthalpy change on freezing of 1.0 mol of water at 10.0^(@)C to ice at -10.0^(@)C . Delta_("fus")H=6.03 kJ mol^(-1) at 0^(@)C C_(p)[H_(2)O(l)]=75.3 J mol^(-1)K^(-1) C_(p)[H_(2)O(s)]=36.8 J mol^(-1)K^(-1)

The enthalpy change on freezing of 1 mol of water at 5^(@)C to ice at -5^(@) C is (Given Delta_("fus") H = 6 kJ mol^(-1) at 0^(@) C , C_(p) (H_(2) O , l) = 75.3 J mol^(-1) K^(-1) , C_(p) (H_(2) O , s) = 36.8 J mol^(-1) K^(-1))